Chemistry, asked by pragnasree6065, 11 months ago

How many grams of CO2 and grams of H2O are produced when 52.0 g C2H2 burns in oxygen?

Answers

Answered by AmritRaaj
105

2C2H2 + 5O2 --> 4CO2 + 2H2O

1 mole of C2H2 = 2 (12.0) + 2(1.0) = 26.0 g

1 mole of CO2 = 12.0 + 2 (16.0) = 44.0 g

1 mole of H2O = 2(1.0) + 16.0 = 18.0 g

52 g C2H2 x 1 mol / 26 g = 2.0 mol C2H2

2.0 mol C2H2 x 4 CO2 / 2 C2H2 = 4.0 mol CO2

4.0 mol CO2 x 44.0 g / mol = 176 g CO2

52 g C2H2 x 1 mol / 26 g = 2.0 mol C2H2

2.0 mol C2H2 x 2 H2O / 2 C2H2 = 2.0 mol H2O

2.0 mol H2O x 18.0 g / mol = 36 g H2O

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Answered by roshnirajeevsl
0

Answer:

88 grams of CO₂ and 36 grams of H₂O are produced when 52.0 g of C₂H₂ burns in oxygen.

Explanation:

Molar mass of C₂H₂ = 12×2 + 1×2

                                 = 26 g/mol

The number of moles is calculated by using the formula,

n = given mass/molar mass

The number of moles of C₂H₂= 52/26

                                                 = 2 moles

2 moles of C₂H₂ ⇒ 4 moles of CO₂.

The molar mass of carbon dioxide is 44 g/mol.

Mass of CO₂ = 44×4  

                     = 176 g

2 moles of C₂H₂ ⇒ 2 moles of H₂O.

The molar mass of water is 18 g/mol.

Mass of H₂O = 18×2  

                     = 36 g

Thus, 176 grams of CO₂ and 36 grams of H₂O are produced when 52.0 g of C₂H₂ burns in oxygen.

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